Science Year 10

Mr Hem’s Class

The Years Topics

• Introduction to the Atom – Chemistry Basics• Climate Change – Will we perish?• STELR – Will we run out of energy?• Chemistry – How are things made? • Evolution – Where did we come from?• Palaeontology – Jurassic Park!• Genetics – How am I so attractive?• QUESTIONS ABOUT SCIENCE (2-3 Qs)

S.MORRIS 2006

HISTORY OF THE ATOM

460 BC Democritus develops the idea of atoms

he pounded up materials in his pestle and

mortar until he had reduced them to

smaller and smaller particles which he

calledATOMA

(greek for indivisible)

HISTORY OF THE ATOM

1808 John Dalton

suggested that all matter was made up of

tiny spheres that were able to bounce

around with perfect elasticity and called

themATOMS

HISTORY OF THE ATOM

1898 Joseph John Thompson

found that atoms could sometimes eject a

far smaller negative particle which he

called an

ELECTRON

HISTORY OF THE ATOM

Thompson develops the idea that an atom was made up of electrons scattered unevenly within an elastic sphere surrounded by a soup of positive charge to balance the electron's charge

1904

like plums surrounded by pudding.

PLUM PUDDINGMODEL

HISTORY OF THE ATOM

1910 Ernest Rutherford

oversaw Geiger and Marsden carrying out his famous experiment.

they fired Helium nuclei at a piece of gold foil which was only a few atoms thick.

they found that although most of them passed through. About 1 in 10,000 hit

HISTORY OF THE ATOM

gold foil

helium nuclei

They found that while most of the helium nuclei passed through the foil, a small number were deflected and, to their surprise, some helium nuclei bounced straight back.

helium nuclei

HISTORY OF THE ATOM

Rutherford’s new evidence allowed him to propose a more detailed model with a central nucleus.

He suggested that the positive charge was all in a central nucleus. With this holding the electrons in place by electrical attraction

However, this was not the end of the story.

HISTORY OF THE ATOM

1913 Niels Bohr

studied under Rutherford at the Victoria University in Manchester.

Bohr refined Rutherford's idea by adding that the electrons were in orbits. Rather like planets orbiting the sun. With each orbit only able to contain a set number of electrons.

Bohr’s Atom

electrons in orbits

nucleus

HELIUM ATOM

+N

N

+-

-

proton

electron

neutron

Shell

What do these particles consist of?

ATOMIC STRUCTURE

Particle

proton

neutron

electron

Charge

+ ve charge

-ve charge

No charge

1

1

nil

Mass

ATOMIC STRUCTURE

the number of protons in an atom

the number of protons and neutrons in an atom

He2

4 Atomic mass

Atomic number

number of electrons = number of protons

ATOMIC STRUCTUREElectrons are arranged in Energy Levels

or Shells around the nucleus of an atom.

•first shell a maximum of 2 electrons

•second shell a maximum of 8 electrons

•third shell a maximum of 18 electrons

•Fourth shell a maximum of 32 electronsNOTE!!! No shell can fit more than 8 electrons unless the

outer electronics have at least 2

ATOMIC STRUCTURE

There are two ways to represent the atomic

structure of an element or compound;

1. Electronic Configuration

2. Dot & Cross Diagrams

Nucleus

X

XX

X

X

X

XX

X

X

XX

X

X

X

X

X

X

X

X

X

X

X

X

X

X

X

X

X

X

X

X

X

X

X

XXX

X

X

X X

ELECTRONIC CONFIGURATION

With electronic configuration elements are represented numerically by the number of electrons in their shells and number of shells. For example;

NNitrogen

7

14

2 in 1st shell 5 in 2nd shell

configuration = 2 , 5

2 + 5 = 7

ELECTRONIC CONFIGURATION

Write the electronic configuration for the following elements;

Ca O

Cl Si

Na20

40

11

23

8

17

16

35

14

28B 11

5

a) b) c)

d) e) f)

2,8,8,2 2,8,1

2,8,7 2,8,4 2,3

2,6

DOT & CROSS DIAGRAMS

With Dot & Cross diagrams elements and compounds are represented by Dots or Crosses to show electrons, and circles to show the shells. For example;

Nitrogen N XX X

X

XX

X N 7

14

DOT & CROSS DIAGRAMS

Draw the Dot & Cross diagrams for the following elements;

O Cl8 17

16 35a) b)

O

X

XX

X

X

X

X

X

Cl

X

X

X

X X

XX

X

X

X

X

X

X

XX

X

X

X

SUMMARY1. The Atomic Number of an atom = number of protons in the nucleus.

2. The Atomic Mass of an atom = number of Protons + Neutrons in the nucleus.

3. The number of Protons = Number of Electrons.

4. Electrons orbit the nucleus in shells.

5. Each shell can only carry a set number of electrons.

Over to You Questions

• Science For Life Book!• Pg. 28 • Chapter 2• Questions 1) 2) 7) 8)a) b) c) • 9) 10) 11) 12) 13) 17)